In this worksheet, we will practice calculating the proportion of particles, in an ideal gas, that have a given speed using the Maxwell–Boltzmann distribution function.
An incandescent light bulb is filled with neon gas. The gas that is in close proximity to the element of the bulb is at a temperature of K. Determine the root-mean-square speed of neon atoms in close proximity to the element. Use a value of 20.2 g/mol for the molar mass of neon.
- A m/s
- B m/s
- C m/s
- D m/s
- E m/s
Helium atoms in a gas that is at a temperature have a root-mean-square speed of 196 m/s. When the gas is heated until it becomes a plasma with a temperature , the root-mean-square speed of the helium atoms is 618 km/s. Use a value of 4.003 g/mol for the molar mass of helium.
- A K
- B K
- C K
- D K
- E K
Using the approximation for small , estimate the fraction of nitrogen molecules at a temperature of K that have speeds between 290 m/s and 291 m/s. A nitrogen molecule has a mass of kg.
In a sample of a monatomic gas, a number of molecules have speeds that are within a very small range around the root-mean-square speed of atoms in the gas, . A number of molecules have speeds that are within the same very small range around a speed of . Determine the ratio of to .
A sample of nitrogen is at a temperature of K. has a molar mass of 28.00 g/mol.
What is the most probable speed of the nitrogen molecules?
What is the average speed of the nitrogen molecules?
What is the root-mean-square speed of the nitrogen molecules?